Chemistry
High School (9–10)
General
The Periodic Table › Development of the Periodic TableThe Periodic Table › Periodic TrendsThe Periodic Table › Groups and FamiliesStructure of the Atom › Electronic Configuration and ValencyChapter 9Contains Standard contentThe Periodic Table
There are more than a hundred elements. How can anyone remember them all? A chemist does not. A chemist reads the periodic table, a chart that puts each element where its properties are easy to guess. In this chapter we see how the first lists were made, how Mendeleev left gaps for elements that nobody had found, and how the modern table is built on the electrons of an atom. Then we use the table to predict size, valency, reactivity and the nature of oxides. Python helps us to test the patterns.
Part of Chemistry · High School (9–10) (chapter 9)
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From Triads to the Modern Table
Why did chemists need a table? In this course we follow the story from Dobereiner's triads and Newlands' octaves to Mendeleev's table with its gaps, and then to the modern table, which is arranged by atomic number.
Patterns Across Periods and Down Groups
Why does carbon make four bonds and oxygen two? Why is a sodium atom bigger than a chlorine atom? In this course we find the valency, the size, the metallic character and the oxides of the elements, and how they change across a period and down a group.